Write balanced ionic equations for the following reactions. (a) Aqueous hydrobromic acid is neutralized by aqueous calcium hydroxide.

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Identify the reactants and products: Hydrobromic acid (HBr) and calcium hydroxide (Ca(OH)_2) react to form water (H_2O) and calcium bromide (CaBr_2).

Write the balanced molecular equation: 2 HBr(aq) + Ca(OH)_2(aq) → 2 H_2O(l) + CaBr_2(aq).

Dissociate all strong electrolytes into their ions: HBr and Ca(OH)_2 are strong electrolytes, so they dissociate completely in water.

Write the complete ionic equation: 2 H^+(aq) + 2 Br^-(aq) + Ca^2+(aq) + 2 OH^-(aq) → 2 H_2O(l) + Ca^2+(aq) + 2 Br^-(aq).

Cancel out the spectator ions (ions that appear on both sides of the equation): The Br^- and Ca^2+ ions are spectator ions, so the net ionic equation is 2 H^+(aq) + 2 OH^-(aq) → 2 H_2O(l).

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주요 개념

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Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this case, hydrobromic acid (HBr) acts as the acid, while calcium hydroxide (Ca(OH)2) serves as the base. The products of this reaction are water (H2O) and calcium bromide (CaBr2), illustrating the fundamental principle of acid-base chemistry.

Ionic Equations

Ionic equations represent the species involved in a chemical reaction in their ionic forms. In aqueous solutions, strong acids and bases dissociate completely into their ions. For the neutralization of hydrobromic acid and calcium hydroxide, the balanced ionic equation will show the ions that participate in the reaction, allowing for a clearer understanding of the chemical changes occurring.

Balancing Chemical Equations

Balancing chemical equations is essential to ensure that the number of atoms for each element is the same on both sides of the equation, adhering to the law of conservation of mass. In the case of the neutralization reaction, it is important to balance the number of hydrogen, bromine, calcium, and oxygen atoms to accurately represent the stoichiometry of the reaction.